A chemist measures the volumes of 1.00 mol CF4 and of 1.00 mol CH3Cl and finds that they differ by 0.20 L at STP conditions
A) Which gas produced the larger volume and why?
B) Do the results contradict the ideal gas law? Why or why not?
C) Rank the volume relative to 22.4L and relative to each other. Were their volumes both above 22.4L? Or would they be below, or maybe you'd think one is over and one is under? Briefly explain your decision.
A) Which gas produced the larger volume and why?
B) Do the results contradict the ideal gas law? Why or why not?
C) Rank the volume relative to 22.4L and relative to each other. Were their volumes both above 22.4L? Or would they be below, or maybe you'd think one is over and one is under? Briefly explain your decision.
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A) CF4 because it's a nonpolar compound, thus the only intermolecular force between each molecule is the london dispersion force, whereas CH3Cl is a polar molecule, therefore it has dipole-dipole forces as well as lond dispersion forces; because the van der waal forces (it forms weak bonds between molecules) of CH3Cl is greater than that of CF4, CH3Cl occupy less volume than CF4 under STP
B) the results contradict the ideal gas law because the law states that any gas under STP occupies a volume of 22.4 liters, and the experiment shows that the two gases differ in volume.
C) the two gases that are closes to being ideal are He and H2, due to their relatively small mass and small size; because both CF4 and CH3Cl are heavy and large compared to those He and H2, their volume are going to be over 22.4 L
B) the results contradict the ideal gas law because the law states that any gas under STP occupies a volume of 22.4 liters, and the experiment shows that the two gases differ in volume.
C) the two gases that are closes to being ideal are He and H2, due to their relatively small mass and small size; because both CF4 and CH3Cl are heavy and large compared to those He and H2, their volume are going to be over 22.4 L